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PORTAGE LEARNING / CHEM 103 / MODULE 3 TO 6
EXAM – 200 HIGH-YIELD QUESTIONS WITH VERIFIED
ANSWERS & DETAILED RATIONALES | 2025/2026 LATEST
UPDATE | GRADED A+
COMPETENCY DOMAINS
• Domain 1: Thermochemistry, Calorimetry & Enthalpy (Module 3)
• Domain 2: Gas Laws & Kinetic Molecular Theory (Module 3)
• Domain 3: Chemical Formulas, the Mole Concept & Percent Composition (Module 4)
• Domain 4: Empirical & Molecular Formulas, Molarity & Dilution (Module 4)
• Domain 5: Chemical Reactions, Balancing & Reaction Types (Module 5)
• Domain 6: Precipitation, Solubility & Net Ionic Equations (Module 5)
• Domain 7: Acid-Base, Redox & Oxidation Numbers (Module 5)
• Domain 8: Stoichiometry, Limiting Reactants, Solutions & Colligative Properties (Modules 5–6)
INTRODUCTION
This comprehensive examination is designed to assess the knowledge, skills, and competency of
candidates preparing for the Portage Learning CHEM 103 General Chemistry I Module 3–6
Examinations. The assessment evaluates essential competencies across core domains through
multiple-choice, calculation-based, and scenario-based questions. Candidates must demonstrate
critical thinking, analytical skills, and mathematical reasoning required to apply chemical
principles effectively in problem-solving and professional practice.
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1. Which of the following best defines an exothermic reaction?
A. A reaction that absorbs heat from the surroundings
B. A reaction that releases heat into the surroundings
C. A reaction in which the temperature of the system decreases
D. A reaction in which ΔH is positive
☑ Correct Answer: B
☑ Explanation: Exothermic reactions release energy, usually as heat, and have a negative
enthalpy change (ΔH < 0). Endothermic reactions absorb heat and have a positive ΔH.
2. In the equation q = mcΔT, what does the variable c represent?
A. Heat capacity of the calorimeter
B. Specific heat capacity of the substance
C. Concentration of the solution
D. Number of moles
☑ Correct Answer: B
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☑ Explanation: c is the specific heat capacity—the amount of heat required to raise the
temperature of 1 gram of a substance by 1°C. It is an intensive property unique to each material.
3. Calculate the heat required to raise the temperature of 25.0 g of water by 12.0°C. (Specific
heat of water = 4.184 J/g·°C)
A. 1,255 J
B. 1,255 kJ
C. 125.5 J
D. 4.184 J
☑ Correct Answer: A
☑ Explanation: q = m × c × ΔT = 25.0 g × 4.184 J/g·°C × 12.0°C = 1,255.2 J ≈ 1,255 J. The other
options reflect incorrect calculations or unit errors.
4. A 50.0 g sample of metal absorbs 1,170 J of heat, and its temperature rises from 22.0°C to
47.0°C. What is the specific heat of the metal?
A. 0.936 J/g·°C
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B. 1.07 J/g·°C
C. 23.4 J/g·°C
D. 0.468 J/g·°C
☑ Correct Answer: A
☑ Explanation: q = mcΔT → c = q/(mΔT) = 1,170 J/(50.0 g × 25.0°C) = 0.936 J/g·°C. The other
options reflect calculation errors.
5. Which statement correctly describes an endothermic process?
A. The system releases heat to the surroundings, and ΔH is negative.
B. The system absorbs heat from the surroundings, and ΔH is positive.
C. The temperature of the surroundings increases.
D. The process always occurs spontaneously.
☑ Correct Answer: B
☑ Explanation: Endothermic processes absorb heat (ΔH > 0), causing the surroundings to
cool. Exothermic processes release heat (ΔH < 0) and warm the surroundings.
PORTAGE LEARNING / CHEM 103 / MODULE 3 TO 6
EXAM – 200 HIGH-YIELD QUESTIONS WITH VERIFIED
ANSWERS & DETAILED RATIONALES | 2025/2026 LATEST
UPDATE | GRADED A+
COMPETENCY DOMAINS
• Domain 1: Thermochemistry, Calorimetry & Enthalpy (Module 3)
• Domain 2: Gas Laws & Kinetic Molecular Theory (Module 3)
• Domain 3: Chemical Formulas, the Mole Concept & Percent Composition (Module 4)
• Domain 4: Empirical & Molecular Formulas, Molarity & Dilution (Module 4)
• Domain 5: Chemical Reactions, Balancing & Reaction Types (Module 5)
• Domain 6: Precipitation, Solubility & Net Ionic Equations (Module 5)
• Domain 7: Acid-Base, Redox & Oxidation Numbers (Module 5)
• Domain 8: Stoichiometry, Limiting Reactants, Solutions & Colligative Properties (Modules 5–6)
INTRODUCTION
This comprehensive examination is designed to assess the knowledge, skills, and competency of
candidates preparing for the Portage Learning CHEM 103 General Chemistry I Module 3–6
Examinations. The assessment evaluates essential competencies across core domains through
multiple-choice, calculation-based, and scenario-based questions. Candidates must demonstrate
critical thinking, analytical skills, and mathematical reasoning required to apply chemical
principles effectively in problem-solving and professional practice.
,2
1. Which of the following best defines an exothermic reaction?
A. A reaction that absorbs heat from the surroundings
B. A reaction that releases heat into the surroundings
C. A reaction in which the temperature of the system decreases
D. A reaction in which ΔH is positive
☑ Correct Answer: B
☑ Explanation: Exothermic reactions release energy, usually as heat, and have a negative
enthalpy change (ΔH < 0). Endothermic reactions absorb heat and have a positive ΔH.
2. In the equation q = mcΔT, what does the variable c represent?
A. Heat capacity of the calorimeter
B. Specific heat capacity of the substance
C. Concentration of the solution
D. Number of moles
☑ Correct Answer: B
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☑ Explanation: c is the specific heat capacity—the amount of heat required to raise the
temperature of 1 gram of a substance by 1°C. It is an intensive property unique to each material.
3. Calculate the heat required to raise the temperature of 25.0 g of water by 12.0°C. (Specific
heat of water = 4.184 J/g·°C)
A. 1,255 J
B. 1,255 kJ
C. 125.5 J
D. 4.184 J
☑ Correct Answer: A
☑ Explanation: q = m × c × ΔT = 25.0 g × 4.184 J/g·°C × 12.0°C = 1,255.2 J ≈ 1,255 J. The other
options reflect incorrect calculations or unit errors.
4. A 50.0 g sample of metal absorbs 1,170 J of heat, and its temperature rises from 22.0°C to
47.0°C. What is the specific heat of the metal?
A. 0.936 J/g·°C
, 4
B. 1.07 J/g·°C
C. 23.4 J/g·°C
D. 0.468 J/g·°C
☑ Correct Answer: A
☑ Explanation: q = mcΔT → c = q/(mΔT) = 1,170 J/(50.0 g × 25.0°C) = 0.936 J/g·°C. The other
options reflect calculation errors.
5. Which statement correctly describes an endothermic process?
A. The system releases heat to the surroundings, and ΔH is negative.
B. The system absorbs heat from the surroundings, and ΔH is positive.
C. The temperature of the surroundings increases.
D. The process always occurs spontaneously.
☑ Correct Answer: B
☑ Explanation: Endothermic processes absorb heat (ΔH > 0), causing the surroundings to
cool. Exothermic processes release heat (ΔH < 0) and warm the surroundings.
